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1. IOSR Journal of Applied Chemistry (IOSR-JAC)
e-ISSN: 2278-5736. Volume 3, Issue 5 (Jan. – Feb. 2013), PP 55-61
www.iosrjournals.org
Reduction of Eu3+ and Doping the Same into Calcium
Thiocyanate Dihydrate Using a Modified Jones Reductor
Dr. (Mrs.) Danja Bertha Abdu
Department of Chemical Sciences, Faculty of Science, 1Federal University Kashere, Gombe State Nigeria
Abstract: The reduction of Europium (Eu³+) in aqueous solution and doping Eu²+ obtained into the host lattice
Ca(SCN)2۰ 2H2O solution using a Modified Jones reductor is described here . The major goal is to dope Eu2+
into compounds that are difficult to dope through the melt method. Ca(SCN)2۰ 2H2O was obtained by the
reaction of Ca(OH)2 and NH4SCN with slow heating at 70oC 0.05% M of EuCl3 was used as the source of Eu
ions. The host lattice was held in the receiver of the modified Jones Reductor, the solution of EuCl3 is slowly
passed through the reductor at the rate of ≈ 0.4 –0.6ml/min under inert gas. The dried sample was prepared in a
glove box for luminescence measurement.
Ca(SCN)2۰ 2H2O:Eu2+ shows an intensive luminescence in the green spectral region. The emission
spectra obtained in this work are all due to the f-d transitions of the Eu2+ ions, a small band due to Eu3+ was
observed, The excitation spectra were measured at 80K at an emission of 19608cm-1 (510nm). A broad almost
shapeless band was observed due to transitions to 4f65d1 states of Eu2+. The modified Jones Reductor was
successfully used to reduce and doped europium into thermally unstable Host lattice.
Keywords: Calcium thiocyanate , Emission spectra, Europium, Excitation spectra, Host lattice, luminescence ,
Modified Jones Reductor, Reduction
I. Introduction
Increasing interest in the chemistry of lanthanides (Ln) has been noticed during the last two decades.
Among the lanthanides, europium (Eu) seems to be the most popular due to the luminescent and catalytic
properties of its complexes, and stability of the 2+ oxidation state. Amongst the Lanthanides, it is only the
element Europium (Eu), ytterbium (Yb) and samarium (Sm) that have significant chemistry (i.e. based on true
Ln2+) in this oxidation state.
A few methods are available for the reduction of lanthanides such as chemical reduction; example is
the effect on the rate of reduction by Zn in HCl medium [2]. Selin et al [3] applied γ-irradiation to reduced Eu
(III) to Eu (II) in aqueous solution of a mixture of rare earth elements. In another work Seln et al also used the
method of radiolytic reduction [4] in dilute aqueous solution. They observed that the reduction of Eu (III) was
enhanced by the presence of Sm3+. Electrolytic reduction of Eu (III) in acidic chloride solutions with titanium
cathode was used by Hirato et al [5] to examine the feasibility of the rare earth separation. They claimed to
achieved complete reduction of 0.1mol of EuCl3(aq) solution. But they observed that the final percent Eu(III)
reduction of the solution from an industrial europium purification process which contained other rare earths, was
lower than that of a synthetic EuCl3 single electrolyte solution.
Polarographic reduction of europium ions on mercury-drop electrode in the presence of halide ions
was used by Levitskaya et al [6] to determine the amounts of europium in Eu-base alloys. In 1987 Kaneko et al
used a method similar to what is being used in this work i.e reduction of europium using zinc fixed beds [7] to
separate europium from other rare earth metals. They passed their solution in the fixed bed for five hours at
2.4L/h rate and obtained 97% reduction. Electrochemical reduction as applied by Marina using nitrates,
bromides and iodide media [8]. Among the elements of the lanthanides group, Eu3+ is characterised by its ability
to be reduced to a bivalent state in aqueous solutions rather easily, even as compared to Sm 3+ and Yb 3+. It is this
property of europium, to be reduced in aqueous solution that is being exploited in this work, because Eu 2+ plays
an important role in luminescence sciences as it has emissions consisting of a 4f7 – 4f65d1 transition which is
parity allowed and thus, very intensive.
Many host lattices have been investigated such as oxides, chlorides and some pseudohalogens. But
thiocyanates are receiving attention as host lattice only of recent, among them Strontium Thiocyanate
(Sr(SCN)2) and Barium Thiocyanate (Ba(SCN)2) have been doped with Eu2+ and measured [9]. It has been
reported that the unusual surrounding of these thiocyanates causes quite a common and very intense green
emission of the Eu2+ [10]. Calcium Thiocyanate (Ca(SCN)2) is considered to be an appropriate host lattice, but
it decomposes at about 420°C and begins to melt at 408.8°C. This implies that decomposition begins
immediately after melting. This makes it difficult to dope Ca(SCN) 2 and other similar compounds with Eu²+
using solid-state reaction, since they are not thermally stable.
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2. Reduction Of Eu3+ And Doping The Same Into Calcium Thiocyanate Dihydrate Using A Modified
The aim of this study is to exploit how Eu³ + can be reduced in aqueous solution and to attempt to dope Eu² + in
Ca(SCN)2 in solution using a Modified Jones Reductor.
II. Material and Methods
Calcium thiocyanate dihydrate was obtained by the reaction of Ca(OH) 2 and NH4SCN with slow heating at
70oC according to reference [9]. To avoid the problem due to oxides in commercial compounds, the Ca(OH) 2
was prepared by the reaction of CaCl2 with NaOH. The equations of the reactions are given in equations 1 and 2
below.
CaCl2 (aq) + 2NaOH (aq) → Ca(OH)2 ( s ) + 2NaCl (aq) (1)
Ca(OH)2 + 2NH4SCN Heating Ca (SCN)2•2H2O + 2NH3↑ + H2O
 (2)
EuCl3 was used in this work as the source of Eu ion. 0.05% M of EuCl 3 in respect to the host lattice
was dissolved in water and used for the reduction. The water used was degassed by boiling it up to expel O 2 and
then nitrogen gas bubbled into it before use. All the chemicals, substances and equipments used are given in
Table 1 and 2 below. Two methods were tried as follows; doped Eu3+ into the host lattice then pass it through
the Jones reductor, the second method was to hold the host lattice in the receiver and reduced only the Eu 3+, then
allow it flow into the receiver containing the host lattice. The second method was found to be better and it was
carried out as follows: The host lattice was held in the receiver, which was dipped into a beaker containing
water. The water was slowly heated to 60 oC with stirring to allow for uniform temperature distribution on the
receiver. One arm of the receiver was connected to inert gas (N 2) and one to vacuum. Before the solution of
EuCl3 was put into the reductor, the arm connected to inert gas was opened to float the system with N 2 so as to
expel O2. The flow of the inert gas was maintained during the reduction. The solution was then slowly passed
through the reductor at the rate of ≈ 0.4 –0.6ml/min. After the completion of the reduction, the arm to inert gas
was closed and that to vacuum opened. The doped compound was slowly evaporated to dryness under vacuum;
this takes one to two days. The dried sample was removed under inert gas, closed and taken into the glove box
and prepared for luminescence measurement.
Table 1: Equipments Used
Equipment Company
Argon glove box Braun [Germany]
Fluorolog®-3 spectrofluorometer, FL3-22 Jobin Yvon [USA]
Liquid nitrogen cryostat, VNF-100 Janis research [Wilmington, MA]
Powder diffractometer D5000 Siemens [Germany]
Imaging Plate Diffraction System, IPDS STOE [Darmstadt, Germany]
IFT-IR Spectrometer, IFS 113V Bruker [Karlsruhe, Germany]
Vacuum Pump ILMVAC GmbH [Germany]
Detector PSD- 50M Braun München Germany
Table 2: Chemicals and Substances Used
Name Formula Purity (%) Supplier
Calcium Chloride CaCl2 p.a Alfa
Sodium Hydroxide NaOH 95 J.T Baker
Ammonium Thiocyanate NH4SCN 98.5 Merck
Europium (III) Chloride EuCl3 99.9 Chempur
Nitrogen gas N2 Uni-Siegen
The X-ray powder diffraction was measured using a D5000-diffractometer shown in fig 1. Fat and film were
used in the sample holder preparations. CuK 1 (  = 154pm) Ge was used as irradiation source. The used
detector was a PSD- 50M from company Braun (München). The sample was always grinded to fine powder. A
small amount of the film was cut, put on one of the sample holder part and a very little amount of fat was
applied before the sample was introduced to the film, after which the whole assembly were put into the big
sample holder. The prepared sample holder was put into the diffractometer and the measurement run using a
computer.
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3. Reduction Of Eu3+ And Doping The Same Into Calcium Thiocyanate Dihydrate Using A Modified
figure 1: X-Ray Powder Diffractometer (D5000)
The luminescence measurement was done using a Fluorolg-3 (FL3-22) spectrofluorometer fig 2. This
spectrofluorometer is equipped with a 450w xenon lamp, two double grated monochromators for emission and
excitation. It also contains a photomultiplier with a photon counting system. The measurement procedure is as
follows: The cryostat was evacuated for about 15minutes and then floated with N2 gas, then cooled down to 80K
using liquid nitrogen cryostat. After cooling the heater was started and the sample intensity adjusted to obtain
maximum intensity possible. Two spectra were measured from the Jones Reductor results, they were then
analysed using DATAMAX computer program and the obtained spectra drawn using another computer program
called Origin. During measurement emission spectra was corrected for the photomultiplier sensitivity and
excitation spectra corrected for the intensity of the excitation source.
figure 2: Fluorolg-3 (FL3-22) Spectrofluorometer
III. Results and Discussion
3.1) Preparation of Calcium Thiocyanate Dihydrate (Ca(SCN)2۰2H2O)
The structure of Ca(SCN)2 has already been solved [2]. The prepared compound was tested for the
phase purity by measuring the X-ray powder diffraction pattern which fit into the dihydrate pattern as presented
in fig 3. This confirmed that the host lattice used was pure phase of Ca(SCN)2.2H2O. This host lattice is very
hygroscopic; therefore the preparations were always done in a glove box.
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4. Reduction Of Eu3+ And Doping The Same Into Calcium Thiocyanate Dihydrate Using A Modified
figure 3: X-Ray powder diffraction of Ca(SCN)2۰2H2O
3.2) Degree of Conversion of Eu3+ TO Eu2+
Two spectra were measured from the Jones Reductor results; Fig 4 below shows the first one. The
emission was obtained at 80K by exciting at 24390cm -1 (400nm). The emission shows a broad band with the
maximum at 19685cm-1 (508nm), which is due to transition from 4f65d1 to 4f7 of Eu2+. The peak has full width
at half maximum Г = 1362cm-1. A second peak can be seen at 14317cm-1 which can be assigned to the f-f
transition of Eu3+. The Eu2+ had relative intensities of 2731292cps and that of Eu3+ was 175403cps.
6 1 7 2+
4f 5d 4f (Eu )
Intensity
3+
f-f(Eu )
16000 18000 20000 22000
-1
Wavenumbers(cm )
figure 4: Emission Spectra of Ca (SCN)2۰2H2O:Eu2+ (First Result from Jones Reductor) Vex = 23923cm-1, T =
80K
Figs 5 below are spectra from the second result of the Jones reductor. The broad band due to f-d transition of
Eu2+ with maximum at 19685cm-1 (508nm) was still observed in the emission spectra. A second peak is
observed at 16260cm-1 (615nm) due to the f-f transition of Eu3+. It may be seen here that the peak due to Eu3+ is
smaller compared to the first, suggesting only very small Eu 3+ still remain.
The result of the reduction of Eu3+ using the Jones reductor is in good agreement with previous
literature findings. Shpigun et al [10] used a flow- in system to reduce and measure Eu3+. Their system made it
possible to avoid the problem of handling europium (II) after reduction, because reduction and determination
were performed in closed flow-injection system. The implication is that detecting this unstable oxidation state
should be done within less than 30seconds after its formation in solution. Their results showed a conversion
degree of europium (III) to europium (II) at a flow rate of 0.4 to 0.6ml/min to be optimum.
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5. Reduction Of Eu3+ And Doping The Same Into Calcium Thiocyanate Dihydrate Using A Modified
-1
19685cm
6 1 7
4f 5d 4f
2+
(Eu )
Intensity
-1
16260cm
3+
f-f,Eu
16000 20000 24000 28000 32000
-1
Wavenumbers(cm )
figure 5: Emission and excitation Spectra of Ca(SCN)2۰2H2O:Eu2+. (Second reduction from Jones
reductor) vex = 24390cm-1, Vem = 19608cm-1, T = 80K
When they used metal solutions prepared in 0.1M HCl, the degree of reduction was 75%, but in 0.25M HCl the
degree of reduction was up to 95%. In this work this much of HCl cannot be used as the Cl- ion will interfere
with the luminescence property of the phosphor. Although here the detection of Eu 2+ was not done within 30
seconds after reduction, it may be suggested that 96% reduction was obtained as calculated from reduction done
in the construction of the Jones Reductor. 0.1M HCl was used to dissolved EuCl3, which was further diluted
with 50ml of water, therefore in comparison with Shpigun et al results only a very dilute acid was used here.
Equally only a small amount (0.05%) of the EuCl 3 salt was used, as such the reduction done here was for a
dilute solution of the europium salt. This could account for the high percentage of reduction in comparison with
their result. One can account for the presence of some Eu 3+ in two ways. One possibility is re-oxidation
considering the long time gap between reduction and measurement. The second possibility is that the reduction
was not complete, only some percentage was reduced and a small percentage remains in solution.
3.3) Luminescence of Ca(SCN)2•2H2O:Eu2+ .
The reduction and doping of 0.05% Eu2+ into the above mentioned host lattice were done several times
to obtain maximum results. Among the two methods mentioned in the experimental section, reducing Europium
in solution and doping it after reduction produced better result. The first method of doping the EuCl3 into the
Host Lattice in solution before passing it into the Jones reductor was not successful. This was because after the
reduction, no Eu2+ could be detected in the thiocyanate. This could be explained by the fact that only very small
amount of Eu3+ (0.05%) was used and this could be shielded from the reducing metal by the thiocyanate.
Ca(SCN)2۰2H2O:Eu2+ shows an intensive luminescence in the green spectral region at low temperature because
of the energetically low lying 4f65d1 state. The green luminescence is shown in fig 6. The emission spectra
obtained in this work are all due to the f-d transitions of the Eu2+ ions, as already mentioned above. Apart from
the band due to Eu3+, only one band is observed for the 4f65d1 →4f7 transition of the Eu2+. This shows that all
Eu2+ ions occupy identical sites; this is expected since there is only one crystallographically distinct Ca 2+ ion.
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6. Reduction Of Eu3+ And Doping The Same Into Calcium Thiocyanate Dihydrate Using A Modified
figure 6: Green luminescence of Ca(SCN)2۰2H2O:Eu2+.
Ca(SCN)2۰2H2O melt at a very low temperature (60oC), as such attempt was made to dope Eu2+ into it by the
melt. The spectra from the melt are very comparable to that obtained from the Jones reductor, only without
traces of Eu3+. Fig 7 shows the spectra obtained by the melt at 100oC. The emission was obtained by exciting at
25000cm-1 (400nm). The emission spectrum shows a broad band with a maximum at 19685cm -1 (508nm) and
full width at half maximum Г = 1535cmcm -1, which is quite similar to that obtained from the Jones Reductor.
Since Ca(SCN)2۰2H2O decomposed at a very low temperature, complete doping could not be achieve, only a
small quantity was used for the doping, as such the green luminescence as obtained from the Jones Reductor
doping could not be obtained for the one through the melt.
The ligands (SCN) in this host lattice are covalent. It is known that for increasing covalence the
interaction between the electrons is reduced since they spread out over wider orbital. Consequently, electronic
transitions between energy levels with an energy difference which is determined by electron interaction shift to
lower energy for increasing covalence (Nephelauxetic effect). This effect shifts the centre of gravity to lower
energy, hence shifting the lowest excited 5d(7F0) state to lower energy. Since the excited d state depends very
strongly on the host lattice, this emission is therefore influenced by the Ca2+ surrounding. Another factor that
could lead to broadening of emission band is the nature of the substance used. This happens when powder is
been handled, because external and internal surface are different. In this case the Eu2+ near the surface
experience a covalence and a crystal field which differs from the bulk and can lead to spectra broadening. In this
work the host lattice is crystal, hence the amount of covalence is the main factor of influence.
6 1 7
4f 5d 4f
Intensity
16000 18000 20000 22000 24000 26000 28000 30000 32000
-1
Wavenumbers(cm )
figure 7: Emission and Excitation Spectra of Ca(SCN)۰2H2O:Eu2+(doped from the melt), T = 80K, Emission
Max = 19685cm-1, Vex = 25000cm-1, Vem = 19230cm-1
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7. Reduction Of Eu3+ And Doping The Same Into Calcium Thiocyanate Dihydrate Using A Modified
The excitation spectra in figure 5 and 7 were measured at 80K at an emission of 19608cm -1 (510nm). A
broad almost shapeless band is observed due to transitions to 4f65d1 states of Eu2+. The lowest excited state is
split to five levels due to the C2 point symmetry. The first excitation maximum, taken from fig 7 is at 22862cm-
1
. All the three emission bands shown above are not completely Gaussian shaped, but rather nearly symmetrical
with a sharp drop on the high energy side. This suggest the stoke shift should not be extremely large, implying
that the change in the metal-ligand distance in the ground and excited state is not very large. The stoke shift
calculated from fig 7 using the maximum of the emission and the first maximum of the excitation band is
3084cm-1. Transitions to the individual 7FJ states of the 4f65d1 levels are not well resolved. But the excitation
band from the melt shows a bit of resolving of these states. The fact that these states are not well resolved only
proves that the exchange interaction between the six 4f6 electrons and the 5d1 electron is large. This is expected
for thiocyanates host lattice.
IV. Conclusion
The following conclusions can be made from the results obtained in this work.
The modified Jones Reductor was successfully used to reduce Eu3+ in solution to Eu2+ and doping the same into
thermally unstable Host lattice, namely Ca(SCN)۰2H2O, but from the Luminescence of Ca(SCN)2•2H2O:Eu2+
measured the problem of re-oxidation due to the long time needed must be addressed. The Modified Jones
Reductor provides a good solution for doping Eu2+ into thermally unstable host lattice.
Acknowledgement
The authors acknowledge all the assistance gotten during this research from the Inorganic working
group II under Prof. Wickleder of the University of Siegen Germany.
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